Question
In: Chemistry
Consider this reaction: A(g) + B(g) C(g) at 298K. Consider the following conditions: What can be said...
Consider this reaction:
A(g) + B(g) C(g) at 298K.
Consider the following conditions:
What can be said about the spontaneity of this reaction compared to the same at standard conditions?
A) It is less spontaneous, but still nonspontaneous overall
B) It is more spontaneous, and is a spontaneous reaction at these conditions
C) It is more spontaneous, but still not spontaneous overall
D) It is less spontaneous, and it is a spontaneous reaction at these conditions
E) It doesn't matter if the conditions change. This reaction is not spontaneous at these conditions, and it can't be compared to standard conditions
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
1.) Consider this exothermic reaction: A(g) + B(g) 2 C(g) + D(g) What can be said...
1.) Consider this exothermic reaction:
A(g) + B(g) 2 C(g) + D(g)
What can be said about the spontaneity of this reaction?
A) It is never spontaneous
B) Not enough info
C) It is only spontaneous at high temperatures
E) It is only spontaneous at low temperatures
F) It is always spontaneous
2.) Consider this reaction:
A(g) + B(g) C(g)
What can be said about the entropy () of this reaction?
A.) It is equal to zero
B) It is...
The following reaction can occur at 298K under appropriate conditions. 2SO2(g) +O2(g)-----> 2SO3(g) An equilibrium mixture...
The following reaction can occur at 298K under
appropriate conditions.
2SO2(g) +O2(g)-----> 2SO3(g)
An equilibrium mixture contain O2(g) and SO3(g) at partial pressure
of 0.50atm and 2.0atm respectively. Using data available in
Appendix 4 of your textbook, determine the equilibrium partial
pressure of SO2 in the mixture. Will this reaction be most favored
at a high or at a low temperature, assuming standard conditions?
Justify your reasoning
Substance.
delta
H°
S°
SO2(g)
-297.
248
SO3(g)
-396.
257
O2(g)
0.
205
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the
equilibrium concentrations of A, B, and C for each of the following
different values of Kc. Assume that the initial concentration of A
in each case is 1.0 M and that the reaction mixture initially
contains no products. Make any appropriate simplifying
assumptions.
-------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------
Part A
Kc= 1.8
Express your answer using two significant figures. Enter your
answers numerically separated by commas.
------------------------------------------------------------------------------------------------------------------------------------------------------------------------
Part B
Kc= 1.0×10−2
Express your answer using two significant...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the
equilibrium concentrations of A, B, and C for each of the following
different values of Kc. Assume that the initial concentration of A
in each case is 1.0 M and that the reaction mixture initially
contains no products. Make any appropriate simplifying
assumptions.
Part A: Kc= 1.0 Express your answer using two
significant figures. Enter your answers numerically separated by
commas.
Part B: Kc= 2.0×10−2 Express your
answer using two significant figures. Enter...
Consider the following reaction: CO2(g)+CCl4(g)⇌2COCl2(g) Calculate ΔG for this reaction at25 ∘C under these conditions: PCO2=...
Consider the following reaction:
CO2(g)+CCl4(g)⇌2COCl2(g)
Calculate ΔG for this reaction at25 ∘C under these
conditions:
PCO2= 0.140 atm
PCCl4 = 0.170 atm
PCOCl2= o.740 atm
ΔG∘f for CO2(g) is −394.4kJ/mol, ΔG∘f for CCl4(g) is
−62.3kJ/mol, and ΔG∘f for COCl2(g) is −204.9kJ/mol.
Express the energy change in kilojoules per mole to one decimal
place.
Consider the following reaction which is at equilibrium at 100°C: A(g) + B(g) ↔ AB (g)...
Consider the following reaction which is at equilibrium at
100°C: A(g) + B(g) ↔ AB (g) ΔH=420 kJ/mol Predict the direction
where the reaction would proceed, and explain your reasoning: a.
The reaction vessel were pressurized to 5atm with helium b. The
temperature were increased to 200°C c. The reaction were coupled
with another reaction: AB + D2 → AD + BD d. The volume of the
reaction vessel were increased from 2.0L to 5.0L without removing
any gas e....
Consider the reaction: CO2(g)+CCl4(g)⇌2COCl2(g). Calculate ΔG for this reaction at 25 ∘C under these conditions. PCO2=...
Consider the reaction: CO2(g)+CCl4(g)⇌2COCl2(g). Calculate ΔG
for this reaction at 25 ∘C under these conditions. PCO2= 0.115 atm
PCCl4= 0.170 atm PCOCl2= 0.760 atm
For the reaction A(g) + B(g) + C(g) " D(g) the following data were obtained at 25°C....
For the reaction
A(g) + B(g) + C(g) "
D(g) the following data were
obtained at 25°C.
Exp’t
Initial [A] (M)
Initial [B] (M)
Initial [C] (M)
Initial Rate (mole∙L–1s–1)
1
0.0500
0.0500
0.0100
6.25 x 10–3
2
0.1000
0.0500
0.0100
1.25 x 10–2
3
0.1000
0.1000
0.0100
5.00 x 10–2
4
0.0500
0.0500
0.0200
6.25 x 10–3
5
0.2000
0.3000
0.3000
?????
Which choice gives correct kinetics information for this
reaction? Which choice is closest to the rate
constant for this...
Consider the reaction A(g)+B(g)->C(g) For which Kc=1.30*102 Assume that .406 mole C(g) is placed in a...
Consider the reaction
A(g)+B(g)->C(g)
For which Kc=1.30*102
Assume that .406 mole C(g) is placed in a cylinder. The
temperature is 300 K and the barometirc pressure on the piston
(which is assumed to be massless and frictionless) is constant at
1.00 atm. The original volume (before the C(g) begins to decompose)
is 10.00 L. What is the volume of the container at equilibrium?
What is the reaction A(g) + B(g) + C(g)------------> D(g) Experiment Initial [A] (mol/L) Initial [B]...
What is the reaction A(g) + B(g)
+ C(g)------------> D(g) Experiment Initial [A] (mol/L) Initial
[B] (mol/L) Initial [C] (mol/L) Initial rate (M/s) 1 0.0500 0.0500
0.0100 6.25*^(-3) 2 0.1000 0.0500 0.0100 1.25*^(-2) 3 0.1000 0.1000
0.0100 5*10^(-2) 4 0.0500 0.0500 0.0200 6.25*10^(-3)
1) What is the order with respect
to each reactant?
2) Write the rate law
3) Calculate K (using the data
from experiment 1)
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